Question

Given the folloiwng two half-reactions: Fe3+ (aq) + 3 e− --> Fe (s)             E0 =...

Given the folloiwng two half-reactions:

Fe3+ (aq) + 3 e− --> Fe (s)             E0 = −0.036 V

Mg2+(aq) + 2 e− --> Mg (s) E0 = −2.37 V

Calculate cell potential (Ecell) for a voltaic cell when [Fe3+] = 1.0 *10-3 M, [Mg2+] = 2.50 M at 25 oC

Hint: (1) Write the overall redox reaction and count the number of electrons transferred; (2) determine the cell potential for a voltaic cell; (3) Calculate Q; (4) Plug in the values into Nernst equation.

-2.26 V
2.26 V
2.33 V
-2.33 V
2.40 V

Homework Answers

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
A voltaic cell employs the reaction: 2Fe+3 (aq) + 3Mg (s) -> 2Fe (s) + 3Mg+2...
A voltaic cell employs the reaction: 2Fe+3 (aq) + 3Mg (s) -> 2Fe (s) + 3Mg+2 (aq) Calculate the Ecell at 25 degrees C under each of the following conditions. Fe+3 + 3e- -> Fe , Ered = -0.036 V 1. [Fe3+] = 1.00 M ; [Mg2+] = 1.00 M 2. [Fe3+] = 2.50 M ; [Mg2+] = 1.8x10-3 M Please show the work, thank you!
What is the cell potential for the spontaneous concentration cell with the reaction Fe3+(aq) + Fe(s)...
What is the cell potential for the spontaneous concentration cell with the reaction Fe3+(aq) + Fe(s) → Fe(s) + Fe3+(aq), with concentrations of Fe3+ of 0.873M and 0.342M at a temperature of 310. K? Ecell = E°cell −(RT/nF)lnQ
A voltaic cell employs the following redox reaction: 2Fe3+(aq)+3Mg(s)→2Fe(s)+3Mg2+(aq) Calculate the cell potential at 25 ∘C...
A voltaic cell employs the following redox reaction: 2Fe3+(aq)+3Mg(s)→2Fe(s)+3Mg2+(aq) Calculate the cell potential at 25 ∘C under each of the following conditions. Part A: [Fe3+]= 1.3×10−3 M ; [Mg2+]= 2.95 M Part B: [Fe3+]= 2.95 M ; [Mg2+]= 1.3×10−3 M
A voltaic cell employs the following redox reaction: 2Fe3+(aq)+3Mg(s)→2Fe(s)+3Mg2+(aq) Calculate the cell potential at 25 ∘C...
A voltaic cell employs the following redox reaction: 2Fe3+(aq)+3Mg(s)→2Fe(s)+3Mg2+(aq) Calculate the cell potential at 25 ∘C under each of the following conditions. Part B: [Fe3+]= 1.6×10−3 M ; [Mg2+]= 3.30 M Part C: [Fe3+]= 3.30 M ; [Mg2+]= 1.6×10−3 M
A voltaic cell employs the following redox reaction: 2Fe3+(aq)+3Mg(s)→2Fe(s)+3Mg2+(aq) Calculate the cell potential at 25 ∘C...
A voltaic cell employs the following redox reaction: 2Fe3+(aq)+3Mg(s)→2Fe(s)+3Mg2+(aq) Calculate the cell potential at 25 ∘C under each of the following conditions. A)   [Fe3+]= 3.05 M ; [Mg2+]= 2.5×10−3 M
A voltaic cell employs the following redox reaction: 2Fe3+(aq)+3Mg(s)→2Fe(s)+3Mg2+(aq) Calculate the cell potential at 25 ∘C...
A voltaic cell employs the following redox reaction: 2Fe3+(aq)+3Mg(s)→2Fe(s)+3Mg2+(aq) Calculate the cell potential at 25 ∘C under each of the following conditions. 1. [Fe3+]= 2.3×10−3 M ; [Mg2+]= 2.90 M Express your answer in units of volts. 2. [Fe3+]= 2.90 M ; [Mg2+]= 2.3×10−3 M Express your answer in units of volts.
A voltaic cell employs the following redox reaction: 2Fe3+(aq)+3Mg(s)→2Fe(s)+3Mg2+(aq) Calculate the cell potential at 25 ∘C...
A voltaic cell employs the following redox reaction: 2Fe3+(aq)+3Mg(s)→2Fe(s)+3Mg2+(aq) Calculate the cell potential at 25 ∘C under each of the following conditions. Part B [Fe3+]= 1.2×10−3 M ; [Mg2+]= 3.25 M Express your answer in units of volts. Part C [Fe3+]= 3.25 M ; [Mg2+]= 1.2×10−3 M Express your answer in units of volts.
Consider the half reactions below. Cu 2+ (aq) + 2 e- -----> Cu (s) Eo =...
Consider the half reactions below. Cu 2+ (aq) + 2 e- -----> Cu (s) Eo = 0.34 V MnO4 - (aq) + 4 H+ (aq) + 3 e- -----> MnO2 (s) + 2 H2O (l) Eo = 1.68 V A. What is the standard cell potential for a voltaic cell comprised of these two half reactions? B. What is the equilibrium constant for this reaction at 25 oC? C. How is the magnitude of the equilibrium constant consistent with a...
4a. Use the Nernst equation to calculate the cell voltage (E) for the following redox reaction:...
4a. Use the Nernst equation to calculate the cell voltage (E) for the following redox reaction: i. Fe3+(aq)+Cu(s)→Cu2+(aq)+Fe2+(aq), given that [Fe3+]=0.05 and [[Cu2+]=0.125M at 25°C, and Fe3++e→Fe2+             E0=0.77 V Cu2+2e→Cu                   E0=0.34 V 4b. Use the information provided in question 4a to calculate the change in free energy (ΔG) and change in entropy (ΔS) for the redox reaction: i. Fe3+(aq)+Cu(s)→Cu2+(aq)+Fe2+(aq) What do the ΔG and ΔS values indicate about the spontaneity of the redox reaction?
Consider the reaction Mg(s)+Fe2+(aq)→Mg2+(aq)+Fe(s) at 69 ∘C , where [Fe2+]= 3.00 M and [Mg2+]= 0.210 M...
Consider the reaction Mg(s)+Fe2+(aq)→Mg2+(aq)+Fe(s) at 69 ∘C , where [Fe2+]= 3.00 M and [Mg2+]= 0.210 M . Part A What is the value for the reaction quotient, Q, for the cell? Part B What is the value for the temperature, T, in kelvins? Part C What is the value for n? Part D Calculate the standard cell potential for Mg(s)+Fe2+(aq)→Mg2+(aq)+Fe(s) Part E For the reaction 2Co3+(aq)+2Cl−(aq)→2Co2+(aq)+Cl2(g).  E∘=0.483 V what is the cell potential at 25 ∘C if the concentrations are [Co3+]=...